The formation of ionic bonds between elements from Group I (alkali metals) and Group VII (halogens) occurs through a transfer of electrons. Alkali metals have one valence electron in their outermost shell, while halogens require one more electron to complete their outermost shell and achieve a stable electron configuration.
Let's take the example of sodium (Na) from Group I and chlorine (Cl) from Group VII to illustrate the formation of an ionic bond. Sodium has one valence electron, while chlorine requires one electron to complete its outer shell.
In a dot-and-cross diagram, sodium is represented by the symbol Na, with a dot next to it representing its single valence electron. Chlorine is represented by the symbol Cl, with seven dots around it representing its seven valence electrons.
To form an ionic bond, sodium will transfer its single valence electron to chlorine. This results in sodium losing one electron to become a positively charged sodium ion (Na+), as it now has one less electron than protons. Chlorine, on the other hand, gains the electron from sodium, resulting in a negatively charged chloride ion (Cl-), as it now has one more electron than protons.
In the dot-and-cross diagram, the electron transfer is represented by an arrow from sodium to chlorine, indicating the movement of the electron. The final configuration shows the sodium ion (Na+) with no dots around it, indicating the loss of its valence electron, and the chloride ion (Cl-) with eight dots around it, representing the complete octet in its outermost shell.
The resulting sodium ion and chloride ion are held together by the strong electrostatic attraction between the oppositely charged ions. This attraction forms an ionic bond, creating an ionic compound known as sodium chloride (NaCl), commonly known as table salt.
This process of electron transfer and formation of ionic bonds occurs between elements from Group I and Group VII, leading to the creation of stable compounds with full outer shells for both elements.
♥️
